CHE154-H KCHE154 S20 Ch17 Sec5-6 Chapter 17 Multiple Choice Question 41 Part A Find the percent ionization of a 0.337 M HF solution. The K, for HF is 6.8 x 104. O4.5 % 1.5 % 6.5% 2.3 x 102 % 6.8 x 102 % Submit Request Answer Provide Feedback
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- Trial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1)Use Kb, the number of moles of C8H4O4^2- at the equivalence point, and the total volume at that point to calculate the pH for each sample at the equivalence point. Compare these calculated results with the experimental results.Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2 given here.a. Ka1 = 1.0 * 10-4; Ka2 = 5.0 * 10-5b. Ka1 = 1.0 * 10-4; Ka2 = 1.0 * 10-5c. Ka1 = 1.0 * 10-4; Ka2 = 1.0 * 10-6Calculate the contributions to [H3O+] from each ionization step. At what point can the contribution of the second step be neglected?The dissociation of 0.15 M phosphoric acid is given by:H3PO4(aq) + H2O(l) ⇄ H2PO4^-(aq) + H3O^+(aq) Ka = 7.1 x 10-3 (at 25°C) H2PO4^-(aq) + H2O(l) ⇄ HPO4^2-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) HPO4^2-(aq) + H2O(l) ⇄ PO4^3-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) A. Classify the species, H3PO4, H2PO4-, HPO4^2-, PO4^3-, as acid, base, or ampholyte.B. Applying the systematic method in solving acid-base equilibria problems, calculate the pH of the following:a. 0.050 M H3PO4 b. 0.050 M NaH2PO4 c. 0.050 M Na2HPO4d. 0.050 M Na3PO4
- The dissociation of 0.15 M phosphoric acid is given by: H3PO4(aq) + H2O(l) ⇄ H2PO4^-(aq) + H3O^+(aq) Ka = 7.1 x 10-3 (at 25°C) H2PO4^-(aq) + H2O(l) ⇄ HPO4^2-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) HPO4^2-(aq) + H2O(l) ⇄ PO4^3-(aq) + H3O^+(aq) Ka = 6.3 x 10-8 (at 25°C) B. Applying the systematic method in solving acid-base equilibria problems, calculate the pH of the following: a. 0.050 M H3PO4 b. 0.050 M NaH2PO4 c. 0.050 M Na2HPO4 d. 0.050 M Na3PO4Determine the pHpH of an HNO2HNO2 solution of each of the following concentrations. Part A 0.510 MM Express your answer to two decimal places. pHpH = nothing SubmitRequest Answer Part B 0.110 MM Express your answer to two decimal places. pHpH = nothing SubmitRequest Answer Part C 1.40×10−2 MM Express your answer to two decimal places. pHpH = nothing SubmitRequest Answer Part D In which cases can you not make the simplifying assumption that x is small? In which cases can you not make the simplifying assumption that x is small? only in (b) only in (a) in (b) and (c) in (a) and (b) SubmitRequest Answer Provide Feedback Next15. A 300.00 mL solution of 0.00165 M A2B5 is added to a 230.00 mL solution of 0.00380 M C2D3. What is pQsp for A2D5?
- Explain why the conductivity of mixture A is higher than that of mixure B, , yet the pH of A is lower than the pH of B. Include relevant equations in your answer B 0.1 mol L–1 CH3COOH Conductivity (mA) 5 PH 3 A 0.1 mol L–1 HCl 260 1Determine the initial concentrations of the species below, after the solutions are mixed. Volume0.0350 MKMnO4(mL) Volume0.0650 MH2C2O4(mL) VolumeH2O(mL) InitialConcentrationKMnO4(M) InitialConcentrationH2C2O4(M) (3 significant figures) (3 significant figures) 1.00 1.00 18.00 2.00 2.00 16.00 3.00 3.00 14.00 4.00 4.00 12.00 5.00 5.00 10.00Calculate the concentration of SCN in each of the following standard solutions. Use 0.0500 M Fe3+ and 0.00200 M SCN- a. 1.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL) b. 2.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL) c. 3.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL) d. 4.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL)
- Give only typing answer with explanation and conclusion to all parts Calculate the concentrations of all species in a 0.490 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are ?a1=1.4×10−2 and ?a2=6.3×10−8. [Na+]= [HSO−3]= [OH−]= [SO2-3]= [H2SO3]= [H+]=Solid silver nitrite is slowly added to 125 mL of a sodium cyanide solution until the concentration of silver ion is 0.0523 M. The maximum amount of cyanide remaining in solution is M. Please post the answer asap please make sure the answer doesnot contain error becasue last answer provided had error so i need to resubmit the question. Thanks!Sample containing arsenic weighing 0.800 are titrated with a standard iodine soluton. what should be the normality of the iodine in order that each ml of titrant represents 1/2% As2O3 in the sample (Answer: 0.0809 N show full solution please)